1. NOTE: Use the HOME/Pos1 button to return to the table of contents.
The Reaction module
Use Reaction to calculate the thermochemical properties of a species or a chemical reaction.
Reaction accesses only compound type databases.
Note that Reaction assumes all gases to be ideal and ignores expansivities and compressibilities of solids and liquids.
Table of contents
Section 1 Table of Contents
Section 2 Opening the Reaction module
Section 3 Pure substance property calculations (pure Cu)
Section 4 Isothermal standard state reactions (oxidation of copper)
Section 5 Using non-standard states in equilibrium reaction
Section 6 Non-isothermal non-equilibrium calculation (heating of pure (Al))
Section 7 Two phase single component equilibrium (ideal binary system)
Section 8 Variable input amounts in non-isothermal reaction
Section 9 Pidgeon Process for the Production of Magnesium
Section 10 Aqueous applications
Section 11 Complex gases and condensed substances under high pressure
NOTE: Use the HOME/Pos1 button to return to the table of contents.
Reaction 1

2. The Reaction module Click on Reaction in the main FactSage window.2

3. Pure substance property calculations (Pure Cu)
The simplest possible application of the Reaction module is the calculation of thermodynamic properties of a pure substance.
In order to do that the input in the Reactants window is not a balanced reaction but a single line with one substance name.
The properties of this substance are calculated as a function of temperature depending upon the choice of the phase state given in the Reactants window. If a particular phase state is chosen, the properties of this phase are calculated, if the option most stable is used, the phase state that corresponds to the temperature that is used in the calculation is chosen.
A graph is given which shows the Gibbs energy minimum principle in order to determine the most stable state.
Reaction
3.0

4. Reactants window - entry of a species
Add a Product
Reaction has two windows – Reactants and Table
Add a Reactant
Open
New Reaction
Entry of reactant species
Compound databases available
Go to the Table window
Reaction
3.1

5. Table window – calculating thermodynamic properties of a species
Open
Save
New Reaction
Stop Calculation
Summary of the Reactants window entry
A multiple entry for T: min, max and step. This results in the computation of the transition temperatures.
Return to the Reactants window
Reaction
3.2

6. Determination of most stable phase by Gibbs energy minimization
Phase with lowest Gibbs energy is the most stable. J J K K
Points on the solid lines for P = 1 atm are given in column «T» and «G» of the previous figure for copper.
Reaction
3.3

7. Isothermal standard state reactions (oxidation of copper)
The classical use of the Reaction module is the determination of the isothermal reaction properties of a stoichiometric reaction.
From the names of the reactants and products as well as their respective stoichiometric coefficients it is possible to calculate from the data stored in a Compound type database the values for DH, DS, DG, DV, DA and K (the equilibrium constant) as functions of temperature.
The results are shown in a table (but can also be plotted using the Figure module, see Figure Help, section 8).
As an example the reaction 4 Cu + O2 = 2 Cu2O is used.
Reaction
4.0

8. Simple isothermal standard state reaction: oxidation of copper
Entry of an isothermal standard state reaction: 4 Cu + O2 = 2 Cu2O
An alternative way to enter this data is from the Slide Show Examples Directory. Go to the menu bar and click on: File > Directories… > Slide Show Examples and double-click on a file.
Isothermal means same “T” throughout
Non-standard states checkbox is not selected
Reaction
4.1

9. Oxidation of copper at various temperatures
Entry: Tmin=300K, Tmax=2000K and step=300K. Note the transition temperatures.
The equilibrium constant column appears for an isothermal standard state reaction. Note: DGº = -RT lnK . (For the values of the gas constant R, click on the Units menu)
Reaction
4.2

10. Using non-standard states in equilibrium reaction
A more advanced application of the Reaction module is the use of non-standard states for the reactants and/or products of a reaction.
This option permits to fix certain activities or partial pressures of the species and to resolve the equation DG° = -RT ln Keq for a suitable variable.
It is for example possible to fix all activites/partial pressures of the reactants and products and thus fix K, set the equilibrium condition DG=0 and then resolve for the temperature that fits the fixed value of K.
Reaction
5.0

11. Simple chemical equilibrium: non standard state oxidation of copper
aCu(s) = “X”
PO2(g) = “P”
Select non standard state
Standard state reaction: PO2(g) = 1.0 atm aCu(s) = 1.0
Reaction
5.1

12. Specifying an extensive property change to deal with chemical equilibrium
For simple chemical equilibrium:
and DG0 = -RT ln Keq
Table provides DG using:
and
when DG = 0.
For the last entry:
PO2(g) = 10-12
aCu(s) = 1
DG = 0, equilibrium
Reaction
5.2

13. Non-isothermal non-equilibrium calculation (heating of pure (Al))
A further use of the Reaction module lies in the calculation of non-isothermal non-equilibrium balances of the extensive property changes DH, DS, DG, DV, DF for a given reaction.
It is assumed that this reaction does not represent an equilibrium but a complete transition from the reactants to the products. Under this condition it is possible to attribute the reactants one temperature and the products another.
Thus the above mentioned extensive property changes from one state (reactants at reactant temperature) to the other (products at product temperature) can be calculated using data from a Compound type database.
As an example the heating of Al is demonstrated by use of the reaction Al(300K) = Al(T).
Reaction
6.0

14. Heating Al from 300 K to the temperature T
phase transition, Al(s) ® Al(l)
(i.e. fusion) at K
DH°fusion = Tfusion• DS°fusion
= J J
= J
Reaction
6.1

15. Heating Al: setting the graphical display with Figure
1. Click on the menu Figure and select Axes...
2. A dialog box opens and provides you with a choice of axes for the figure you wish to plot.
Reaction
6.2

16. Heating Al: a few thermodynamic considerations
liquid
17.9 kJ
Point the mouse to read the coordinates of the melting point.
solid
933 K
Reaction
6.3

17. Two phase single component equilibrium (ideal binary system)
An thermodynamically more advanced application of the Reaction module is its use in the calculation of the equilibrium of pure solid with its liquid under the assumption that this liquid is dissolved in a solvent (some other liquid which is not explicitely given) under the condition of ideal mixing.
This situation is reflected in an equilibrium of the type:
Me(pure solid,T) = Me (liquid,a(Me) = x(Me),T)
In the example Cu is used. A graph for the phase boundary of the ideal liquid in equilibrium with the pure solid is given.
Reaction
7.0

18. Computation of Cu liquidus in an ideal binary system: data entry
Cu(solid) = Cu(liquid)
aCu(solid)= 1, pure solid copper
aCu(liquid)= X
Your choice of phases:
liquid phase from the FACT database;
2 compound databases are included in your data search.
Reaction
7.1

19. Computation of Cu liquidus in an ideal binary system: database entry
2. Follow the instructions if you want to include or exclude a database in the data search.
1. To connect databases, click on the Data Search menu, select Databases… to open the Databases dialog box.
3. Follow the instructions if you want to add or remove (and this does not delete) a database from your list.
Reaction
7.2

20. For an ideal solution: aCu(liquid) = XCu(liquid)
Computation of Cu liquidus in an ideal binary system: tabular and graphical output
Calculated activity of Cu(liquid) in equilibrium (DG=0) with pure Cu(solid) at various temperatures T.
For an ideal solution: aCu(liquid) = XCu(liquid)
Liquid
Liquidus line
Liquid + Solid
The 2 specified variables, T and DG, are highlighted.
Note: When DG = 0, the reaction must be isothermal.
Reaction
7.3

21. CH4 + (2 + excess) O2 = CO2 + 2 H2O + (excess) O2
Variable input amounts in non-isothermal reaction and autobalance feature
The following example shows how a variable amount for a reactant can be used to simulate an excess of this substance, i.e. its appearance both among the reactants and the products.
As an example the combustion reaction
CH4 + (2 + excess) O2 = CO2 + 2 H2O + (excess) O2
is used. The Alpha variable is introduced to handle the excess amount.
In the example is also shown how the autobalance feature can be used to generate stoichiometric coefficient that satisfy the mass-balances automatically.
Reaction
8.0

22. Combustion of methane in excess <Alpha> O2 – data entry
The reactants are at 298 K but the products are at an unspecified T.
Variable quantity <Alpha>
The phase of each species is specified.
The reaction is non-isothermal (except when T = 298 K). Hence:
Keq will not appear as a column in the Table window.
Setting DG = 0 is meaningless ( except when product T = 298 K).
Reaction
8.1

23. Combustion of methane in excess <Alpha> O2 – adiabatic reactions
Stoichiometric reaction (A = 2): CH4 + 2 O2 = CO2 + 2 H2O
Reaction with excess O2 (A > 2): CH4 + (2 + excess) O2 = CO2 + 2 H2O + (excess) O2
Exothermic reaction
Adiabatic reaction: DH = 0
Product flame temperature
As <A> increases, the flame temperature decreases. Energy is required to heat the excess O2.
Reaction
8.2

24. Heating the products of the methane combustion
Heating the products of the methane combustion. Reaction «auto-balance» feature
Reaction
8.3

25. Step wise heat balance in treating methane combustion
Different thermodynamic paths, same variation of extensive properties (here DH).
2000 K
Overall Process DH = J
Warming Products DH = J
Isothermal Reaction Heat DH = J
298 K
298 K
Reaction
8.4

26. Pidgeon Process for the Production of Magnesium
The following five slides show how various aspects of the Pidgeon process (production of Mg vapor from MgO in a redox reaction with Si) can be treated using reaction thermochemistry.
Reaction
9.0

27. Pidgeon Process for the Production of Magnesium
Apparatus Schema:
Water-cooled vacuum connection also condenses alkalis
1423 K
Equilibrium Mg partial pressure developed at the hot end of the retort
MgO-SiO2 phase diagram:
Note: MgO(s) and SiO2(s) can not coexist.
Reaction
9.1

28. Pidgeon Process for the Production of Magnesium: Data Entry
In the reaction, the hydrostatic pressure above the condensed phases: MgO(s), Si(s) and SiO2(s2) is 1 atm – i.e. has no effect.
The reaction is isothermal (same “T” throughout), hence DG = 0 gives equilibrium.
The activity of SiO2 is: aSiO2= X.
The partial pressure of Mg(g) is: PMg(g) = P atm.
Allotrope s2(solid-2) has been selected for SiO2 in order to fully specify the phase – if the phase is not completely specified, equilibrium calculations (DG = 0) can not be performed.
Reaction
9.2

29. Equilibrium Mg partial pressure developed at the hot end of the retort
Note: There are an infinite number of values of (PMg(g) , aSiO2(s2)) which satisfy Keq . Here we select 3 special cases.
Standard state reaction at 1423 K: PMg eq = 1 atm and aSiO2(s2) = 1 DGº = kJ = -RT ln Keq, hence Keq = × 10-9 DGº > 0 but Mg can be produced by reducing PMg(g) and/or aSiO2.
At equilibrium(DG=0), when aSiO2(s2)=1.0 and T=1423 K, PMg eq= × 10-5 atm
At equilibrium(DG=0), when PMg eq=1atm and T=1423 K, aSiO2(s2) eq= × 10-9
When DG=0, T=1423 K and aSiO2(s2)= then PMg(g) eq= × 10-3 atm. This value of aSiO2(s2) is taken from the next page calculation.
Reaction
9.3

30. Computation of SiO2 activity when MgO coexists with (MgO)2•SiO2
Pure MgO
Pure (MgO)2•SiO2
SiO2(s2) at activity X
Gives the equilibrium value of the activity of SiO2(s2) at 1423 K: aSiO2(s2)=
Isothermal…
…and at equilibrium
Reaction
9.4

31. Alternative way to calculate equilibrium Mg partial pressure
Remember, DG = 0 (equilibrium) calculations are only meaningful for isothermal reactions («T» throughout).
Magnesium production is enhanced by:
reducing the total pressure (< atm);
reducing aSiO2 – this is done automatically due to (MgO)2 SiO2 formation, but the addition of say CaO (slag formation) reduces aSiO2 further.
Reaction
9.5

32. Aqueous applications
In the following two slides examples are given for the use of the Reaction module in aqueous thermochemistry.
It should be noted however, that ideal behaviour of the aqueous species is assumed since Reaction accesses Compound type databases. If a system requires non-ideal behaviour of the aqueous phase the Equilib module must be used.
Reaction
10.0

33. Hydrogen reduction of aqueous copper ion - Reactants and Table windows
The standard Gibbs energy change underlined yields standard reduction potential of Cu2+ when divided by -2 Faradays. (Remember: DG° = -nFEº, where F (= C/mol) is the Faraday constant)
The molality of Cu2+ is given by “X”.
H2(g) pressure is “P” atm.
Standard state reaction at K
Standard state reaction at various temperatures
Equilibrium molality at various PH2
Reaction
10.1

34. Thermal balance for leaching of zinc oxide
The reaction is exothermic: DH < 0.
This entry calculates the product temperature for an adiabatic reaction: DH = 0.
Reaction
10.2

35. Complex gases and condensed substances under high pressure
The following two slides show how Reaction is used on a system with polymer formation in the gas phase (Na(l) ↔ Na1 + Na2) and on a pure substance system that is submitted to very high pressure (C).
Reaction
11.0

36. Computation of Na and Na2 partial pressure in equilibrium with liquid Na
Both reactions are isothermal, hence DG=0 gives equilibrium.
Na(l) ® Na(g) (monomer)
2 Na(l) ® Na2(g) (dimer)
1. Calculate T when PNa = 1 atm
2. Calculate PNa when T = 1158 K
3. Calculate PNa2 when T=1158 K
Na also forms a gaseous dimer Na2(g). The proportion of Na2/Na near the boiling point ( K) of Na is: 0.111/0.888 at 1158 K; and the total vapor pressure over Na(l) would be: PNa + PNa2 ( ).
Reaction
11.1

37. Effect of high pressure on the graphite to diamond transition
Where available, density (i.e. molar volume) data for solids and liquids are employed in REACTION (the “VdP” term) although their effect only becomes significant at high pressures. (However, unlike EQUILIB, compressibility and expansivity data are NOT employed.)
At 1000 K and atm, graphite and diamond are at equilibrium (DG=0)
Here, carbon density data are employed to calculate the high pressure required to convert graphite to diamond at 1000 K.
The volume of diamond is smaller than graphite. Hence, at high pressures, the “VdP” term creates a favorable negative contribution to the enthalpy change associated with the graphite ® diamond transition.
Reaction
11.2